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  • 1. Part 2: Types of Chemical Reactions Objectives For this Lesson
  • 2. Objectives For this Lesson
    • After this lesson you should be able to:
    • 1. Classify a chemical reaction as composition, decomposition, single replacement, or combustion.
    • 2. Predict the products of simple composition and decomposition reactions.
  • 3. Objectives cont.
    • 3. Use the activity series of metals to produce the products of single replacement reactions.
    • 4. Write the products of the double replacement reaction between two ionic compounds.
  • 4. 5 Types of Reactions
    • Composition (synthesis)
    • Decomposition
    • Single Replacement
    • Double Replacement
    • Combustion
  • 5. Composition (synthesis) Reactions
    • Two or more substances react to form a single substance .
    • These reactions usually result in the release of energy .
    A+ B AB S + O O O O S
  • 6. Your Turn
    • Write a balanced chemical equation for the reaction of:
      • solid aluminum with sulfur.
      • Water and dinitrogen pentoxide.
  • 7. Decomposition Reactions
    • A single substance is broken down into two or more substances.
    A+ B AB O O C Ca O O Ca + O O C
  • 8. Try These
    • Write a balanced chemical equation for the decomposition of:
      • Aluminum oxide.
  • 9. Single Replacement Reactions
    • One element displaces another element from a compound in a single replacement reaction.
    A+ BX AX +B Fe + S O O O O Cu S O O O O Fe Cu +
  • 10. Activity Series
    • Whether an element will replace another depends upon how active the elements are. A more active element will replace a less active element.
    • See your activity chart to determine which elements are more active than others.
  • 11. Solving Single Replacement Reactions
    • Determine what is being replaced, the metals or nonmetals.
    • Look up the elements on your activity series chart, to see if the reaction will take place.
    • Write the complete skeleton equation, and balance it.
  • 12. Your Turn
    • Write balanced chemical equations for the reaction of:
      • Potassium and Zinc Chloride.
      • Chlorine and Hydrofluoric acid.
      • Iron and Sodium phosphate.
      • Fluorine and hydrochloric acid.
  • 13. Double Replacement Reactions
    • Two ionic compounds exchange cations and anions.
    • Hint: “outsides combine, insides combine ”.
    AX+ BY AY +BX
  • 14. + + O O N O Ag K Cl Cl Ag O O N O K
  • 15. Try these
    • Write a balanced chemical equation for the reaction of
      • Lithium iodide and silver nitrate.
      • Barium chloride and potassium carbonate.
  • 16. Combustion Reactions
    • A substance burning in oxygen .
    • Combustion reactions usually involve hydrocarbons .
    • Complete combustion results in the formation of water and carbon dioxide.
    • Incomplete combustion results in the formation of soot and carbon monoxide.
  • 17. Examples
    • Write a balanced chemical equation for the complete combustion of Propane, C 3 H 8
    • Write a balanced chemical equation for the incomplete combustion of Propane.